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BONDING - Coggle Diagram

- - - - E.g sulfate SO4 2-
        
        Sulfide S2-
  - - - NO3- nitrate
      - SO4 2- sulfate
      - CO3 2- carbonate
      - NH4 + ammonium
    - - Ionic compounds need to be neutral overall
      - The charges must balance
      - Do Not include charges in the formula
- - - - H-Cl HYDROGEN CHLORIDE
      - H-O-H WATER(H2O)
      - O=O OXYGEN
      - O=C=O CARBON DIOXIDE
      - H2=C=H2 METHANE
      - H-H HYDROGEN
    - - Low boiling/melting points
        
        -DO NOT BREAK THE BOUNDS
        
        All we do is break is the weak intermolecular forces of attraction
      - Poor electrical conductivity
        -There are no charge carriers available to move and carry current (charge carriers=ions or free electrons)
  - - - A lattice made up of covalently bonded atoms
      - There are NO intermolecular forces on a lattice - there are only covalent bonds.
      - E.G. diamond, silicon dioxide and graphite
    - - High melting and boiling point
        
        Poor electrical conductivity(except graphite)
        
        Very strong (except graphite)
    - - Allotropes: different structural forms of an element
      - DIAMOND,GRAPHITE,GRAPHENE=giant covalent
        
        DIAMOND
        
        STRUCTURE:giant covalent lattice.
        
        BONDING: each carbon is covalently bonded to 4 other carbons. -There are NO free electrons.
        
        PROPERTIES: Really strong(strongest natural material) (3D lattice made of strong covalent bonds)
        
        -doesn't conduct electricity because there are no ions or free electrons to carry the current.
        
        -high MP & BP: need to break strong covalent bonds which requires a lot of energy.
        
        USE: jewellery,
        
        -drill bits as the structure of a diamond is very strong
        
        GRAPHITE
        
        STRUCTURE:giant covalent lattice
        
        BONDING:each has 3 bonds to other carbons
        
        PROPERTIES: does conduct electricity-C has 4 outer electrons but only 3 are in bonds. So each carbon has 1 free electrons so they can carry current.
        
        GRAPHENE
        
        One layer of graphite.
        
        PROPERTIES: same as graphite except strength. Graphene is very strong
      - FULLERENES=simple covalent
        
        Unlike all the other allotropes these are simple covalent molecules NOT giant structures.
        
        Fixed formula e.g. C60
        
        Spherical molecular
        
        PROPERTIES: poor conductors of electricity (despite each carbon having 1 free electron)
        
        USE: lubricant
      - EXAM Q
        
        EXAM A
        
        Carbon has 4 outer electrons so diamond which has a giant covalent structure has no electrical conductivity as carbon is covalently bonded to 4 other carbons so there are no free electrons to carry the current. However graphite which also has a giant covalent structure that has for every 1 carbon has 3 bonds to other carbons so each carbon has 1 free electron so they can move and carry current. But this is contradictory to Fullerene being a simple covalent molecule; it has poor conductors of electricity as it can not carry currents from molecule to molecule despite each carbon having 1 free electron as it has for every 1 carbon has 3 bonds to other carbons.